Instructions:

Use quadrille or lined paper $($unless Microsoft Excel is required$)$

Answer questions$/$problems in the order given.

Write paraphrased problem$/$question statements $($given$,$ assume, find$)$

Use explicit dimensional analysis.

Mark final answers.

Separate problems$/$questions clearly.

If possible, please be compact.

For each of the chemical equilibrium shown, answer the following questions:

a$)$ Give the chemical name of the species in the "reactant" and the "product" sides of the equilibrium.

b$)$ Determine the standard Gibbs free energy change of reaction, ${}_{r}G,$ and the equilibrium constants, Keq, for the following reactions using the tabulated values for ${}_{f}G$ in the textbook Appendix.

c$)$ Decide if the reaction happens spontaneously in the direction it is written.

d$)$ Determine if each of the reactions is endothermic or exothermic.

e$)$ Write the expressions for equilibrium constant for each reaction based on activities.

$1\mathrm{.}1H_{2}P{O}_4^{-}(aq)+H^{+}(aq)>H_{3}P{O}_4(aq)$

$($Compare to the related two examples worked in class and provide a sensible comment$)$

Answer: $222\mathrm{.}5k\frac{J}{m}ol,$ Keq$=9\mathrm{.}95$x$10$

$($Compare to the related one worked in class and provide a sensible comment$)$

$1\mathrm{.}3Ca(S{O}_4)(s)>C{a}^{2+}(aq)+S{O}_4^{-2}(aq)$

$1\mathrm{.}4Ca(S{O}_4)**2H_{2}O(s)>C{a}^{2+}(aq)+S{O}_4^{-2}(aq)+2H_{2}O(l)$

$1\mathrm{.}5HAs{O}_4^{-2}(aq)+H^{+}(aq)>H_{2}As{O}_4^{-}(aq)($Answer: $-41\mathrm{.}4k\frac{J}{m}ol)$

$1\mathrm{.}8O_2(g)+H_{2}O(l)>O_2(aq)+H_{2}O$

$1\mathrm{.}9,C{O}_2(g)+H_{2}O(l)>H_{2}C{O}_3(aq)$

Apply and find meaning of the van't Hoff equation. Accompany the calculation with a sensible comment.

$2\mathrm{.}1$ For problems $1\mathrm{.}3$ and $1\mathrm{.}9,$ prepare a table with three columns: T $($Temperature$),$ K $($Equilibrium constant$),$ and $ln(K).$ Show the calculation by hand for two temperatures. Draw a graph of $lnK$ vs $T$ with five points and add a trendline. If you use Excel, submit your file.

$2\mathrm{.}2$ Do the same for Example B$-3)$ solved in class. $($on the last thre slides of ENV$4113\_$M$03\_$Thermodynamic$\_$Basis$\_$Of$\_$Equilibrium$\_$Chemistry.pdf$)$